Chapter 16 Review               =“Solutions               ”     Pre-AP Chemistry  Charles Page High School     Stephen L. ...
Chapter 16 Review If the solubility of a particular solute is  10 g/100 g H2O at 20 oC, which of the  following would rep...
Chapter 16 Review Colligative   properties depend upon  the ____. What happens to the solubility of a  gas in a liquid, ...
Chapter 16 Review The solubility of a gas in a liquid is  ____ proportional to ____. To what concentration variable is  ...
Chapter 16 Review What  factors will usually make a  substance dissolve faster in a  solvent? In a concentrated solution...
Chapter 16 Review What  are the solution concentration  units used to express molarity? What is the maximum amount of  K...
Chapter 16 Review Ifthe percent by volume is 2.0 %  and the volume of solution is 250  mL, what is the volume of solute i...
Chapter 16 Review The  volume of alcohol present in  620 mL of a 40.0 % (v/v) solution of  alcohol is ____. A solute dep...
Chapter 16 Review What  is the boiling point of a  solution that contains 3 moles of  KBr in 2000 g of water? (Kb = 0.512...
Chapter 16 Review What  is the freezing point of a  solution that has 5.0 mol of NaI in  1250 g of water? (Kf = 1.86 oC/m...
Chapter 16 Review What  is the molality of a solution  containing 5.0 mol of solute in 3.2 kg  of solvent? What is the m...
Chapter 16 Review How many liters of a 1.5 M  solution are required to yield 5.0 g  of solute? (molar mass of solute =  3...
Chapter 16 Review If the solubility of a gas is 7.5  g/L at 404 kPa pressure, what  is the solubility of the gas when  th...
Chapter 16 Review What is the number of moles of  solute in a 0.3 molal solution  containing 0.10 kg of solvent? If 1.0 ...
Chapter 16 Review Calculate the molality of a  solution prepared by dissolving  175 g KNO3 in 750 g of water.
Upcoming SlideShare
Loading in …5
×

Chapter 16 review

2,201 views

Published on

Published in: Technology, Business
0 Comments
0 Likes
Statistics
Notes
  • Be the first to comment

  • Be the first to like this

No Downloads
Views
Total views
2,201
On SlideShare
0
From Embeds
0
Number of Embeds
4
Actions
Shares
0
Downloads
13
Comments
0
Likes
0
Embeds 0
No embeds

No notes for slide

Chapter 16 review

  1. 1. Chapter 16 Review =“Solutions ” Pre-AP Chemistry Charles Page High School Stephen L. Cotton
  2. 2. Chapter 16 Review If the solubility of a particular solute is 10 g/100 g H2O at 20 oC, which of the following would represent a supersaturated solution of that solute: a) 9 g/100 g H2O at 20 oC, or b) 11 g/100 g H2O at 20 oC. If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was ____.
  3. 3. Chapter 16 Review Colligative properties depend upon the ____. What happens to the solubility of a gas in a liquid, if the partial pressure of the gas above the liquid decreases? Which of the following substances is less soluble in hot water than in cold water: a) CO2(g), or b) KBr(s)?
  4. 4. Chapter 16 Review The solubility of a gas in a liquid is ____ proportional to ____. To what concentration variable is change in boiling point directly proportional? What usually occurs to solubility as temperature increases? What units are generally used to express solubility?
  5. 5. Chapter 16 Review What factors will usually make a substance dissolve faster in a solvent? In a concentrated solution, there is a ____ amount of solute. What are the three colligative properties of a solution we have studied?
  6. 6. Chapter 16 Review What are the solution concentration units used to express molarity? What is the maximum amount of KCl that can dissolve in 200 g of water at 20 oC? (the solubility of KCl is 34 g/100 g H2O at 20 oC) What does NOT change when a solution is diluted by the addition of more solvent?
  7. 7. Chapter 16 Review Ifthe percent by volume is 2.0 % and the volume of solution is 250 mL, what is the volume of solute in solution? What two factors affect the solubility of a particular substance? Which of the following equations yields the number of moles? a) M x L, or b) M x mass of solution
  8. 8. Chapter 16 Review The volume of alcohol present in 620 mL of a 40.0 % (v/v) solution of alcohol is ____. A solute depresses the freezing point because the solute ____. To increase the solubility of gas at constant temperature from 1.20 g/L at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to ____.
  9. 9. Chapter 16 Review What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (Kb = 0.512 oC/m; molar mass of water = 18 g/mol) What mass of KCl (solubility 34 g/100 g H2O at 20 oC) can dissolve in 3.30 x 102 g of water?
  10. 10. Chapter 16 Review What is the freezing point of a solution that has 5.0 mol of NaI in 1250 g of water? (Kf = 1.86 oC/m; molar mass of water = 18.0 g/mol) How many kilograms of solvent are in a sample of 0.30 molal solution, if the sample contains 13 moles of solute?
  11. 11. Chapter 16 Review What is the molality of a solution containing 5.0 mol of solute in 3.2 kg of solvent? What is the molarity of a solution containing 1.2 g of solute in 450 mL of solution? (molar mass of solute = 24 g/mol) How many liters of a 0.30 M solution are needed to give 2.7 mol of solute?
  12. 12. Chapter 16 Review How many liters of a 1.5 M solution are required to yield 5.0 g of solute? (molar mass of solute = 30.0 g/mol) If the volume of solute is 6.0 mL and the volume of solution is 300.0 mL, what is the solute’s percent by volume?
  13. 13. Chapter 16 Review If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of the gas when the pressure is 202 kPa? What is the number of moles of solute in 650 mL of a 0.40 M solution?
  14. 14. Chapter 16 Review What is the number of moles of solute in a 0.3 molal solution containing 0.10 kg of solvent? If 1.0 mL of 6.0 M HCl is added to 499 mL of water to give exactly a 500 mL solution, what is the molarity of the dilute solution?
  15. 15. Chapter 16 Review Calculate the molality of a solution prepared by dissolving 175 g KNO3 in 750 g of water.

×